Zinc nitride
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| Zinc nitride | ||
|---|---|---|
 | ||
| Identifiers | ||
| CAS number | 1313-49-1  | |
| Properties | ||
| Molecular formula | Zn3N2 | |
| Molar mass | 224.15 g/mol[1] | |
| Appearance | gray powder[1] | |
| Density | 6.22 g/cm³, solid[1] | |
| Solubility in water | insoluble (decomposes) | |
| Structure | ||
| Crystal structure | Cubic, cI80 | |
| Space group | Ia-3, No. 206[1][2] | |
| Hazards | ||
| EU classification | not listed | |
| NFPA 704 |
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(verify) (what is: / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | ||
| Infobox references | ||
Zinc nitride (Zn3N2) is an inorganic compound of zinc and nitrogen. In pure form, it is cubic in structure.[1][2]
Chemical properties
Zinc nitride can be obtained by thermally decomposing zincamide (zinc diamine)[3] in an anaerobic environment, at temperatures in excess of 200 °C. The by-product of the reaction is ammonia.[4]
3Zn(NH2)2 → Zn3N2 + 4NH3
It can also be formed by heating zinc to 600 °C in a current of ammonia; the by-product is hydrogen gas.[3][5]
3Zn + 2NH3 → Zn3N2 + 3H2
Zinc nitride reacts violently with water to form ammonia and zinc oxide.[3][4]
Zn3N2 + 3H2O → 3ZnO + 2NH3
It is soluble in hydrochloric acid[6] and "reversibly reacts with lithium electrochemically".[7] Like magnesium nitride (Mg3N2) and lithium nitride (Li3N), it has a high melting point.[8]
See also
References
- ↑ 1.0 1.1 1.2 1.3 1.4 Sangeeta, D. (1997). Inorganic Materials Chemistry Desk Reference. CRC Press. p. 278. ISBN 978-0-8493-8900-9. Retrieved 2007-09-30.
- ↑ 2.0 2.1 Partin, D. E.; Williams, D. J.; O'Keeffe, M. (1997). "The Crystal Structures of Mg3N2 and Zn3N2". Journal of Solid State Chemistry 132 (1): 56–59. Bibcode:1997JSSCh.132...56P. doi:10.1006/jssc.1997.7407.
- ↑ 3.0 3.1 3.2 Roscoe, H. E.; Schorlemmer, C. (1907) [1878]. A Treatise on Chemistry: Volume II, The Metals (4th ed.). London: Macmillan. pp. 650–651. Retrieved 2007-11-01.
- ↑ 4.0 4.1 Bloxam, C. L. (1903). Chemistry, Inorganic and Organic (9th ed.). Philadelphia: P. Blakiston's Son & Co. p. 380. Retrieved 2007-10-31.
- ↑ Lowry, M. T. (1922). Inorganic Chemistry. Macmillan. p. 872. Retrieved 2007-11-01.
- ↑ Comey, A. M.; Hahn, D. A. (1921). A Dictionary of Chemical Solubilities: Inorganic (2nd ed.). New York: Macmillan. p. 1124. Retrieved 2007-11-01.
- ↑ Amatucci, G. G.; Pereira, N. (2004). "Nitride and Silicide Negative Electrodes". In Nazri, G.-A.; Pistoia, G. Lithium Batteries: Science and Technology. Kluwer Academic Publishers. p. 256. ISBN 978-1-4020-7628-2. Retrieved 2007-11-01.
- ↑ Grolier Incorporated (1994). Academic American Encyclopedia. Danbury, CT: Grolier Inc. p. 202. ISBN 978-0-7172-2053-3. Retrieved 2007-11-01.
Further reading
- Futsuhara, M.; Yoshioka, K.; Takai, O. (1998). "Structural, electrical and optical properties of zinc nitride thin films prepared by reactive RF magnetron sputtering". Thin Solid Films (Elsevier) 322 (1): 274–281. Bibcode:1998TSF...322..274F. doi:10.1016/S0040-6090(97)00910-3.
- Lyutaya, M. D.; Bakuta, S. A. (1980). "Synthesis of the nitrides of Group II elements". Powder Metallurgy and Metal Ceramics (Springer) 19 (2): 118–122. doi:10.1007/BF00792038.
External links
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